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Dynamic Article LinksC<Journal ofMaterials Chemistry
Cite this: J. Mater. Chem., 2011, 21, 7401
www.rsc.org/materials PAPER
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View Article Online / Journal Homepage / Table of Contents for this issue
Preparation of porous composite ion-exchange membranes for desalinationapplication†
Chalida Klaysom,a Roland Marschall,a Seung-Hyeon Moon,b Bradley P. Ladewig,ac G. Q. Max Lu*a
and Lianzhou Wang*a
Received 29th November 2010, Accepted 15th March 2011
DOI: 10.1039/c0jm04142d
Via a two-step phase inversion technique, composite membranes with controllable porosity and
a significant improvement of electrochemical properties were successfully prepared. The presence of
surface functionalized mesoporous silica (SS) as inorganic fillers in the sulfonated polyethersulfone
(sPES) polymer matrix was proved to have a great impact on the resultant membrane structure, which
subsequently led to significantly enhanced ionic conductivity of the membranes. The correlation among
inorganic fillers, composite structures, electrochemical properties and desalination performance by
electrodialysis (ED) was discussed in detail. The optimal membrane was the composite with 0.2 wt% SS
loading, which possessed a good ionic conductivity of 5.554 mS cm�1, a high selectivity with 0.95
transport number while maintaining good mechanical strength and thermal stability. Moreover, the
performance of this membrane in ED was comparable to a commercial membrane (FKE), exhibiting
a current efficiency of 0.84 and 3.82 kW h kg�1 of salt removed.
Introduction
Ion-exchange membranes have attracted great attention from
both academic and industrial fields, due to their versatile
potential applications including water purification and food
processing.1–10 Many attempts have been made by a number of
research groups to develop robust membranes with desirable
properties for different applications. These include (1) a search
for new polymers with highly modified chemical structures
enhancing membrane conductivity and electrochemical proper-
ties, (2) surface and structure modification of existing commer-
cial membranes, and (3) improvement of considerably cheaper
polymer in the market by blending other polymers or incorpo-
rating some additives into the parent matrix.11–13 Though the
concept of combining two distinct materials forming a new
composite that keeps desirable properties of both components
has been well established, it has not been applied much in the
development of ion-exchange membranes especially in desali-
nation applications. In this work we aim to design a new type of
aARC Centre of Excellence for Functional Nanomaterials, School ofChemical Engineering and Australian Institute of Bioengineering andNanotechnology, The University of Queensland, Qld, 4072, Australia.E-mail: [email protected]; Fax: +61 7 3365 4199; Tel: +61 7 3365 4218bGwangju Institute of Science and Technology, School of EnvironmentalScience and Engineering, Gwangju, 500-712, Republic of KoreacMonash University, Department of Chemical Engineering, Vic, 3800,Australia
† Electronic supplementary information (ESI) available: Supplementaryinformation. See DOI: 10.1039/c0jm04142d
This journal is ª The Royal Society of Chemistry 2011
hybrid ion-exchange membranes by introducing inorganic fillers
to the sulfonated polyethersulfone (sPES) polymer matrix.
Sulfonated aromatic hydrocarbons such as sPES have been
extensively used as an alternative electrodriving membrane due
to their low cost, excellent mechanical, thermal and chemical
stabilities. Moreover, this type of polymers is also easy to process
and has been widely used as the polymer matrix alternative in
replacing Nafion for composite membranes in fuel cell applica-
tion.10,14–16 A variety of inorganic fillers such as sulfonated
polyhedral oligomeric silsesquioxane (sPOSS), phosphotungstic
acid, boron phosphate, clay, and silica were introduced into the
sPES to prepare a composite membrane by either sol–gel or
blending method.17–21 A few successful examples of composite
proton-exchange membranes with improved ion-exchange
capacity and conductivity suitable for fuel cell application have
been reported.17–27 For instance, Choi et al. recently reported the
preparation of sulfonated polysulfone/sPOSS fiber composite
membranes with superior ion-exchange capacity and high proton
conductivity even at very low relative humidity.17 Note that this
type of membranes required several steps to prepare, which may
be disadvantageous for scale-up preparation. Despite the success
in composite proton exchange membrane preparation, the
development of composite membranes for desalination applica-
tion has been very rare. In our previous work, composite
membranes containing a small amount of surface functionalized
mesoporous silica (SS) in the sPES polymer matrix were
prepared by a simple procedure. The resultant composite
membranes exhibited enhanced electrochemical properties while
still retaining excellent mechanical strength and thermal
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stability.28 However, due to the dense structure of the obtained
membranes prepared by the widely used solvent evaporation
method, their ionic conductivity was still very low, being
incomparable with commercial membranes on the market.
In the present work, we report an innovative structural
modification pathway, namely the two-step phase inversion
technique, to tailor the membrane porosity of the sPES–SS
composite membranes, which in turn led to significantly
improved ionic conductivity for the membranes. The relationship
among porosity/structure, physicochemical and electrochemical
properties of the resultant membranes was investigated in detail.
Encouragingly, the performance of this new type of membrane in
ED desalination was comparable to that of a commercial FKE
membrane.
Experimental
Material synthesis
The synthesis procedure and material characterization of sPES
and SO3H-functionalized mesoporous SiO2 (SS) were described
in more detail elsewhere.13,28 The ion-exchange capacity of SS
was measured by back titration. The structure and morphology
of the SS were studied by transmission electron microscopy
(TEM, JEOL 1010) and X-ray diffraction (XRD, Rigaku Min-
iflex) under copper radiation (CuKa, 30 kV and 15 mA).
Membrane preparation
Composite membranes were prepared by a two-step phase
inversion procedure. In the first step, a polymer solution con-
sisting of 25 wt% sPES in dimethylformamide (DMF, Sigma)
was prepared, and then various amounts of SS (0–2 wt%) were
added into the polymer solutions at 60 �C for 4 h under stirring.
Sonication was applied to the mixture solution before it was cast
on glass substrates using a doctor blade with a casting thickness
of ca. 0.40 mm. In the second step, the cast film was dried in
a vacuum oven at 60 �C for 10 min and then precipitated in a 60–
70 �CDI water bath. The formed membrane sheet was peeled off
from the glass substrate and kept in DI water. A series of
membranes were named by considering the wt% of SS added into
the polymer matrix. For instance, 0.2SS represents the composite
membrane of sPES containing 0.2 wt% of SS. The prepared
membranes were then treated in hot water for 2 h and then in
1 mol dm�3 HCl for 24 h. Subsequently, the membranes were
rinsed with DI water and kept in 1 mol dm�3 NaCl solution. All
membranes were equilibrated in working solution for at least 6 h
before use.
Membrane characterization
Membrane morphology. Scanning electron microscopy (SEM,
JEOL 6300) was used to observe the morphology and structure
of the prepared membranes. To obtain a sharp cross-sectional
surface the samples were fractured in liquid nitrogen, and then
the captured water was dried out overnight in a freeze dryer to
preserve their structure.
Ion-exchange capacity (IEC) and water uptake of ion-exchange
membranes. Ion-exchange capacities were measured by a back
7402 | J. Mater. Chem., 2011, 21, 7401–7409
titration technique. Firstly, the cation-exchange membrane was
soaked in 1 mol dm�3 HCl for at least 6 h. After that, the
membrane was washed with DI water to remove the excess HCl
and then was immersed into 1 mol dm�3 NaCl solution for
another 6 h. The number of displaced protons from the
membrane was determined by titration with 0.01 mol dm�3
standard NaOH solution using phenolphthalein as an indicator.
Then the membrane was soaked in DI water for 24 h or more.
Afterward, the membrane was taken out and the excess water on
the surface was removed with tissue paper. The wet weight of
membrane was measured. Then the membrane was dried at 50 �Cin an oven for 10 h or until there were no weight changes in the
membranes. The dry weight of the membrane was recorded. The
IEC and water uptake of membranes were then calculated using
eqn (1) and (2):
IEC ¼ ab
Wdry
(1)
Water uptake ¼ Wwet �Wdry
Wdry
(2)
where a is the concentration of NaOH solution (mol dm�3), b is
the volume of NaOH solution used (dm3), Wdry is the dry
weight of the membrane and Wwet is the wet weight of the
membrane.
Electrochemical properties of ion-exchange membranes
Membrane resistance. The resistance of membranes was
measured by impedance spectroscopy (IS) using a Solarton 225B.
The working ion-exchange membrane was equilibrated in
0.5 mol dm�3 NaCl before being placed in a two-compartment
cell between platinum electrodes with an effective area of 1 cm2.
The test was carried out in a frequency range of 1–106 Hz with an
oscillating voltage of 100 mV.29 The resistance corresponding to
the phase angle closest to zero in the Bode diagram was recorded.
Then, the membrane resistance (Rmem) was calculated by
subtraction of the electrolyte resistance (Rsol) from the
membrane resistance equilibrated in the electrolyte solution
(Rcell), according to the equation Rmem ¼ Rcell � Rsol. The
conductivity of membranes (s, S cm�1) was then calculated by
eqn (3):\displaystyle
s ¼ L
RmemA(3)
where Rmem was the resistance of membranes, L is the thickness
of membranes (cm), and A is the effective area of the membranes
(cm2).
Membrane potential and transport number. The membrane
potential was measured with dilute solutions in order to render
negligible the activity coefficient of the electrolyte.30 The
investigated membrane was placed in a two-compartment cell,
separating two NaCl concentration solutions of 0.01 mol dm�3
and 0.05 mol dm�3, respectively. The potential difference (Em)
across the membrane was measured at room temperature using
a multimeter which was connected to two Ag/AgCl reference
electrodes. The transport number, �ti, was calculated by the
following equation:4
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Em ¼ RT
F
�2ti � 1
�ln
�C1
C2
�i
(4)
where R is the gas constant, F is the Faraday constant, T is the
absolute temperature, C1 and C2 are the concentrations of elec-
trolyte solutions in the testing cell, respectively.
Fig. 1 ED cell configuration (a) and schematic diagram of the test in ED
system (b).
Current–voltage (i–v) characteristic and chronopotentiometry.
The i–v curve and chronopotentiogram of the membranes in
0.025 mol dm�3 NaCl were measured at room temperature using
the same two-compartment cell. The cell was connected to
a Solartron Multistat 1480 by two Pt electrodes. For i–v curves,
a stepwise potential difference was applied across the membrane
and the corresponding current was measured. The chro-
nopotentiogram was carried out at a constant applied current
density of 3 mA cm�2 and the corresponding potential was
recorded every 1 s for a period of 300 s automatically.
Thermal and mechanical stabilities of membranes
Thermal stabilities. Thermogravimetric analysis (TGA)
(Mettler Teledo) was used to study the thermal stability of the
membranes in the temperature range of 25–800 �C with a heating
rate of 10 �C min�1 under a nitrogen flow of 20 cm3 min�1.
Mechanical properties. The mechanical properties of wet
membranes were measured by the tensile test at room tempera-
ture using an Instron 5800 at a speed of 2 mm min�1. The tested
samples were equilibrated in DI water for 24 h and then cut into
a rectangular shape with dimensions of 50 mm � 5 mm. The
gauge length of each specimen was 14 mm. At least five speci-
mens from each sample were tested.
Desalination by electrodialysis
The performance of the prepared membranes was tested in
a custom designed ED cell. The cell consists of 5-compart-
ment chamber made of Perspex sheet. Each chamber provides
4 cm2 active area for membranes with an o-ring to prevent
leakage during the testing. The scheme of the ED setup and
the membrane configuration in the cell are illustrated in
Fig. 1.
The ED of NaCl solution was carried out with potentiostatic
modes. The feed solution (150 cm3 of 0.2 mol dm�3 NaCl) was
circulated at 30 cm3 min�1 through the dilute and concentrated
compartments. The concentrated compartments were adjacent to
the electrode rinse compartments in which 150 cm�3 of 3 wt%
Na2SO4 was circulated at 30 cm3 min�1. The commercial cation-
exchange membranes FKE were placed at the positions C1 and
C3 in Fig. 1(a) next to the electrode to separate the electrode
solution from the product solution. The composite membrane as
a cation-exchange membrane was placed in position C2 and
commercial anion-exchange membrane was placed in position A
to complete the cell. The performances of the prepared
membranes were compared with the commercial membrane in
terms of flux, current efficiency and energy consumption calcu-
lated by the following equations.
Flux ¼ DN
At(5)
This journal is ª The Royal Society of Chemistry 2011
h ¼ FzDN
ncÐIdt
(6)
P ¼ FzU
3600hMNacl
(7)
where h ¼ current efficiency of the dilute, F ¼ Faraday constant
(96 487 As mol�1), DN ¼ Cdn�1Vd
n�1 � CdnVd
n (mole), Cd ¼concentration of dilute (mol dm�3), Vd ¼ volume of the dilute
(dm�3), P ¼ power consumption of NaCl (kW h kg�1), nc ¼number of cell pair, I ¼ current (A), U ¼ applied voltage (V),
MNaCl ¼ molecular weight of NaCl (58.45 g mol�1), A ¼ active
surface area (cm2), and t ¼ time (s).
The ion concentration from each compartment was deter-
mined by a conductometer and the pH of solution from each
chamber was measured to indicate the water electrolysis that may
occur during the process. The volume change in each reservoir
was recorded at the start and end of the experiment.
Results and discussion
Structure influence of the inorganic fillers on composite
properties
Following the same procedure in our previous work,22 the SS
with a particle size of 100–150 nm was firstly synthesized. The
highly ordered mesoporous materials were evidenced by TEM
images (Fig. 2(b and c)). Moreover, the small angle XRD of as-
synthesized sulfonated SiO2 showed well resolved reflections of
2D-hexagonal mesostructure with indexes of (100), (110), (200),
and (210), confirming the highly ordered pore structure of the
particles. The ion-exchange capacity of the SS particle was
J. Mater. Chem., 2011, 21, 7401–7409 | 7403
Fig. 2 Small angle XRD patterns (a) and TEM (b and c) images of sulfonated mesoporous silica (SS) at different magnifications.
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estimated to be 1.8 mequiv g�1 by back titration, which is
consistent with those reported in previous works.13,28
The SS particles were first mixed with polymer solution of
sPES and DMF, followed by the two-step phase inversion
process to form membrane sheets.31 FTIR spectrum was used to
investigate the chemical structure of each component and
possible intermolecular interaction. As shown in Fig. S1†, IR
vibration bands at around 1140 and 1205 cm�1, characteristics of
SO3H groups attached to the silica, and at 1030 cm�1 for sulfo-
nate groups of sPES were observed. These indicate the presence
of ion-exchangeable groups in both sPES and SS components.
However, the FTIR bands of the SS could not be clearly iden-
tified in the composite, possibly due to the very small proportion
of SS in the composite or band position overlapping of the
components.32
The morphology of the obtained composites was shown to be
highly porous (Fig. 3). Compared to the pristine membrane, the
presence of additives increased the porosity of the membranes.
Not only the porosity of the membranes increased with SS
loading, but also the pore size of the membrane. At higher
loading the SS particle tends to form clusters, thus resulting in
a bigger pore size. Though the SS cluster formation became more
pronounced at high percentage of SS loading, these primary
Fig. 3 SEM images of (a1 and 2) sPESmembranes, (b1 and 2) composites wit
wt% SS.
7404 | J. Mater. Chem., 2011, 21, 7401–7409
clusters were still well distributed throughout the entire structure
of the polymer matrix.
The key properties of ion-exchange membranes including
water uptake, IEC, conductivity and transport number were
summarized in Table 1. As mentioned earlier, incorporating high
surface functionalized silica was expected to improve the IEC
and water uptake and thus enhances the conductivity and
transport properties of the membranes. The water uptake of the
membrane was significantly improved due to three main effects
of the additives; the additional hydrophilic functional groups
carried by the high surface area SS, the inherit property of silica
to keep both physical and chemically bound moisture, and pore
formation of the membrane contributed by SS, creating free
space to absorb more water.33 Since water channel promotes the
migration of the ionic species, the conductivity of the membrane
increased, following the same trend of the water uptake. Like-
wise, the IEC of the membrane increased with increasing
the loading amount of SS and peaked at low percentage (around
0.2 wt%) of SS. The decrease of IEC when more SS was added
may be due to the interaction among functional groups of the
inorganic filler clusters, because agglomeration of fillers can
cause the loss of the accessibility of the functional groups in SS
and thus the decrease of IEC, resulting in lower water content. In
h 0.2 wt% SS, (c1 and 2) 0.5 wt% SS, (d1 and 2) 1 wt% SS, and (e1 and 2) 2
This journal is ª The Royal Society of Chemistry 2011
Table 1 Physicochemical and electrochemical properties of the prepared membranes compared with commercial membranes
Name Water uptake (%) IEC/mequiv g�1 s/mS cm�1 Transport number Free volume fraction
0SS 38.67 0.75 0.336 0.90 0.4330.2SS 92.00 0.83 5.554 0.95 0.740.5SS 85.00 0.78 1.460 0.95 0.701.0SS 79.00 0.73 1.330 0.96 0.692.0SS 55.00 0.69 0.960 0.91 0.67FKEa 48.10 1.20 3.834 0.95 NA
a A commercial cation exchange membrane from FumaTech, Germany. The FKE is made of sulfonated poly(ether ether ketone). The wet thickness ofthe commercial membrane was 50 � 10 mm which is similar to those prepared membranes.
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addition, more inorganic agglomerate (>1wt% SS) in the
composite means reduced proportion of sPES in the membrane.
Thus the ion-exchangeable functional groups contributed from
sPES could also be reduced. For these reasons, the increased
inorganic fillers and pore cavity did not lead to better membrane
performance. The pore volume or free volume fraction in the
composite membranes again suggests the optimal condition of
0.2 wt% SS, calculated by the following equation:
Free volume fraction ¼ rwet � rdry
rw(8)
where rwet, rdry and rw are the density of wet membrane, dry
membrane and water at room temperature, respectively.
The results of morphology and properties as described earlier
revealed that incorporating inorganic fillers had a significant
impact on the membrane structure which was also directly
related to the properties of the membranes. The influence of these
inorganic fillers was schematically described in Fig. 4. In the
phase inversion process for membrane formation, the final
Fig. 4 Schematic diagram of pore formation with the presence of inorganic
functional groups.
This journal is ª The Royal Society of Chemistry 2011
structure of the membrane is determined largely by the property
of the casting polymer solution and its viscosity.34–37 The less
viscous the polymer solution is, the faster the solvent/nonsolvent
exchange rate is, resulting in a more porous membrane structure.
The pore formation of the composite in the presence of SS may
be attributed to the incompatibility between the inorganic fillers
and the organic polymers, creating a polymer-poor phase. As
a result, the high exchange rate of solvent/nonsolvent around the
inorganic fillers creates pore cavity capturing the SS particles.
When more SS was added in the polymer matrix, the particles
tend to form bigger clusters and thus bigger pores were
produced. It can be seen from the SEM image, at more than 1 wt
% SS loading, the obvious large cavities with pore interconnec-
tion were obtained. When the inorganic fillers formed large
clusters, their surface functional groups were reduced and also
started to interfere with the charged functional groups of the
polymer matrix. As a consequence, the physicochemical and
electrochemical properties of the composite declined after
reaching a maximum value.
fillers and the charge interfering between inorganic clusters and polymer
J. Mater. Chem., 2011, 21, 7401–7409 | 7405
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The thermal and mechanical properties of these membranes
were investigated by TGA and tensile test, respectively (Fig. 5).
Three-step weight loss was observed for the membranes. The first
weight loss at the temperature below 100 �C is associated with the
release of the absorbed moisture. Then, the slight loss at around
280 �C can be assigned to the decomposition of sulfonate
groups,38 and finally dramatic loss occurring at around 500 �C is
due to the degradation of polymer chains. From the TGA curve,
it is observed that the membranes exhibited a better thermal
stability in the presence of inorganic fillers. This may be attrib-
uted to the interaction among the functional groups.
The mechanical testing was carried out under wet conditions
and the results are presented in terms of Young’s modulus,
tensile stress, and strain as shown in Fig. 5(b and c). Incorpo-
rating inorganic fillers enhanced the energy distribution
throughout the membranes, thus the membranes can withstand
more pressure. However, in the presence of additives the
membranes became more elastic and more elongated under
the tensile force. As a consequence, the Young’s modulus of the
membranes decreased. At high degrees of loading, membranes
became more brittle, resulting in the increment of the Young’s
modulus.
For comparison, the thermal and mechanical properties of the
commercial FKE membrane, which is made of sulfonated poly
(ether ether ketone), were acquired from the supplier. It was
informed that the FKE possesses high thermal stability above
270 �C with a Young’s modulus of 1124 MPa, a tensile stress of
36.39 MPa and a tensile strain up to 195.26% at 95% RH.
Compared to the FKE membrane, our prepared membranes
showed comparable thermal stability but lower mechanical
stability. However, one should keep in mind that the testing
conditions from the company and our experiment were different.
The mechanical properties of the commercial membrane were
tested under 95% RH, while our membrane was tested under the
fully hydrated condition. Nevertheless, it was clear to conclude
from the results of this section that our composite membranes
exhibited excellent thermal stability up to 280 �C and decent
mechanical strength up to 600 MPa, which are sufficient for
application in desalination.
Fig. 6 Chronopotentiograms (a) and their derivative potential vs. time
curve (b) of the synthesized membranes compared with commercial
membranes tested at room temperature in 0.025 mol dm�3 NaCl.
Electrochemical behavior of the composite membranes
It is of crucial importance to understand the electrochemical
behavior of the membranes and to predict their performance and
behavior in a real application. The electrochemical behavior of
Fig. 5 Thermal (a) and mechanical properties (b: Young’s m
7406 | J. Mater. Chem., 2011, 21, 7401–7409
as-synthesized membranes was studied utilizing well known
chronopotentiometry and current–potential (i–v) techniques.
Chronopotentiometry is a powerful tool for studying transport
phenomena and concentration polarization near membrane
interfaces. In this work, it was used for investigating the homo-
geneity of membrane surface as the ion-exchange membranes are
generally considered inhomogeneous in the micro-scale consist-
ing of conducting and non-conducting regions. By applying
a constant current density to the system and measuring the
corresponding potential as a function of time, the typical chro-
nopotentiograms with three-stage potential differences were
obtained and shown in Fig. 6(a). After the constant current
density is applied to the system, the concentration polarization
arises, resulting in the concentration gradient and slow increase
of potential at the first stage. When the concentration near the
membrane interface of the depleting solution decreases to nearly
zero, the potential rapidly increases before reaching the steady
state at the end. The time at which the potential transition occurs
is called the transition time (s). The transition time can also be
expressed by the well known Sand’s equation:
s ¼ ðC0ziFÞ2pD4i2ðti � tiÞ2
(9)
where i is the current density, C0 is the concentration of elec-
trolyte, and zi is the valence of the ith ion. It is worth noting that
the eqn (9) was proposed under the assumption of entire con-
ducting surface of the membranes. The s deprived from Fig. 6(b)
odules, c: strain and stress) of the prepared membranes.
This journal is ª The Royal Society of Chemistry 2011
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of the derivative dE/dt at the maximum value where the rapid
potential increase occurred is listed in Table 2 and compared with
the ideal value estimated from eqn (9). It clearly showed the
deviation between those values obtained experimentally and
theoretically. This can be explained by the effects of surface
inhomogeniety of the membranes. Considered ion-exchange
membranes as microheterogeneous membranes with reduced
conducting surface, the local current density at the conducting
regions is higher than the overall current density applied to the
system. As a result, the time required to deplete the ionic species
became shorter. The current density in the conducting region (i*)
was expressed as a function of overall current density or so-called
superficial current density (i) and the fraction of the conducting
region (3) as shown below;
i* ¼ i/3 (10)
And thus the 3 can be estimated by the derived Sand’s equation
given as:
3 ¼ 2is1=2ðti � tiÞC0ziFðpDÞ1=2
(11)
The fraction of conducting surface, 3, including all characteristic
values from chronopotentiograms is summarized in Table 2. The
starting potential (E0) and the potential at the steady state (Emax)
varied in each membrane. These characteristic values are
believed to be dependent on the resistance of membranes and the
testing systems. The fraction of conducting region increased with
the amount of SS added and peaked at 0.2 wt% loading which is
in a good agreement with the result in the previous section. The
results clearly showed that the shape of chronopotentiogram and
their characteristic values are highly influenced by the surface
heterogeneity of the membranes. While the membrane with more
surface heterogeneity (0SS) exhibits more diffused curve with
more interval time (Dt) where the derivative dE/dt is not zero as
can be seen in Fig. 6(b), the more surface homogeneous
membranes with the presence of SS shows more defined transi-
tion time with smaller interval time.
The i–v characteristic was also used to investigate the
concentration polarization of membrane interface and the
limiting operating point so-called the limiting current density
(LCD). By recording the corresponding current density with the
stepwise potential difference, typical i–v curves of the prepared
membranes were obtained as shown in Fig. 7. The linear rela-
tionship of current and potential in the beginning stage followed
the Ohm’s law. Subsequently, a plateau was reached when the
concentration of the dilute solution near the membrane interface
Table 2 Characteristic values from chronopotentiograms
Sample �ti sa/s sb/s 3 E0/V Emax/V Dt/s
0SS 0.90 32.2 24 0 0.864 3.45 3.94 260.2SS 0.95 26.6 26.5 0.997 3.14 3.83 200.5SS 0.95 26.6 26.5 0.997 3.14 3.90 241SS 0.96 25.7 23.0 0.946 3.20 3.93 242SS 0.91 30.9 23.0 0.862 3.25 3.95 19FKE 0.95 26.6 26.0 0.988 3.10 3.94 24
a Estimated from eqn (9). b Deprived experimentally fromchronopotentiogram.
This journal is ª The Royal Society of Chemistry 2011
dropped nearly to zero due to the concentration gradient that
arose from concentration polarization. The LCD can then be
estimated from intersection of the tangents from these two
regions. The corresponding current above the plateau region can
be referred to a ‘‘so-called’’ over-limiting region which was
believed to be influenced dominantly by the convection effects.
The derivative dE/di is deprived from the original i–v curve and
plotted as a function of i and E as shown in Fig. 7(b and c),
respectively, in order to avoid the ambiguous estimation of the
LCD from the ill-defined characteristic curve and to better
visualize the plateau length. According to the concentration
polarization theory, the LCD was expressed in terms of diffusion
boundary layer thickness (d), diffusion coefficient (D), and
transport number as shown in eqn (12):
ilim ¼ jzjCFDd�ti � ti
� (12)
It is clear from the eqn (12) that under the same testing condi-
tions, the LCD depends on the transport number of membrane.
Note that the dwas considered constant in this work as this value
is a function of hydrodynamic property such as feed flow or
stirring rate which was also controlled in the experiment. The
lower the transport number the membrane has, the higher the
LCD of the membrane was expected.
However, the result showed that our composite membranes
with higher transport number possessed the higher LCD. This
may be attributed from the reduced conducting area of the
microheterogeneous membranes explained earlier. The superfi-
cial LCD (i) deprived from Fig. 7(b) and the local LCD (i*) of the
conducting region estimated from eqn (10) were compared in
Table 3. The results showed that the local LCD (i*) is propor-
tional to the reciprocal of the transport number of the
membranes, theoretically expressed in eqn (12). It is also inter-
esting to take a note of the plateau length of the prepared
membranes that decreased with the increase of % loading and the
fraction of the conducting region. The more heterogeneous the
membrane surface is, the longer the plateau length is. This is
consistent with reports in the literature.4,30,39–42 However, the
plateau length of composites with 2 wt% SS was much smaller
than the parent membrane even though they possessed close 3
values and similar properties. This may be explained by the effect
of geometrical heterogeneity reported by early studies,39,40
revealing that not only the fraction value (3) but also the
arrangement and distribution between conducting and non-
conducting regions needed to be taken into account for
explaining the plateau shortening or prolonging behavior. If the
space distance between the two compartments is in the same
magnitude with the boundary-layer thickness, the shortening
plateau length of heterogeneous membranes would also be
observed.
It is clear that the presence of SS fillers improved the con-
ducting fraction of the membrane surface and consequently
improved the LCD and electrochemical behavior.
Desalination of NaCl by ED
The performance of composite membranes with 0.2 and 0.5 wt%
SS in a custom-designed ED cell was evaluated and compared
with the unmodified and commercial membranes. The ED test
J. Mater. Chem., 2011, 21, 7401–7409 | 7407
Fig. 7 i–v curve (a), and derivative dE/di as a function of i (b) and derivative dE/di as a function of E (c) of the obtained membranes measured at room
temperature in 0.025 mole dm�3.
Table 3 Characteristic values from i–v curve
Sample i/mA cm�2 i*/mA cm�2 DE/V
0SS 2.19 2.54 1.600.2SS 2.21 2.21 0.940.5SS 2.04 2.04 0.671SS 2.21 2.33 0.532SS 2.08 2.41 0.70FKE 2.06 2.08 1.10
Table 4 Performance of the prepared membranes compared withbenchmark in ED
Operating E/V SampleFlux/molem�2 h�1 h
P/kW hkg�1 salt
7 0SS 4.56 0.56 5.740.2SS 6.62 0.84 3.820.5SS 6.73 0.79 4.01FKE 7.46 0.83 3.92
5 0.5SS 4.12 0.99 2.28FKE 4.10 0.75 3.11
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was carried out with potentiostatic mode (CV) at 7 volts. The
concentration of desalting solution, pH and current density were
recorded over the testing period and the results were shown in
Fig. 8. The average values over the testing time of flux, current
efficiency and energy consumption were then calculated and
listed in Table 4. The composite membranes showed significantly
better performance compared to the pristine membrane, due to
the remarkable enhanced conductivity and transport properties
by incorporating surface functionalized silica. It is also inter-
esting to note that under the same testing condition, the
composite membranes also show comparable performance to the
benchmark membranes. Unlike the commercial membrane FKE,
which experienced the pH change after 60 min of operation, our
membranes were quite stable and the pH change was observed
Fig. 8 Electrodialysis of NaCl solution: changes of (a) c
7408 | J. Mater. Chem., 2011, 21, 7401–7409
for 0.5 wt% SS after 240 min. To ensure that the pH change was
not because of the chemical degradation of the membranes
during the ED operation, the IR spectra of the membranes
before and after ED testing were investigated (see ESI, Fig. S2†).
It was clear that there were no apparent difference of the
chemical structure observed. This implies that water dissociation
was occurring with the commercial and 0.5SS membranes, an
inappropriate testing condition for these two membranes.
Therefore, the lower potential condition was used for FKE and
0.5SS membrane to avoid water splitting phenomena. The results
are also shown in Table 4. In the later situation, the 0.5SS
membrane performed notably better than the commercial one
with 0.99 current efficiency and 2.28 kW h kg�1 of salts removed.
oncentration, (b) pH and (c) current density vs. time.
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As the performance of ED not only depends on membrane
properties but also the testing conditions and cell design, the
optimal operating condition of a given testing cell should be
carefully tuned.
Conclusion
A new two-step phase inversion membrane formation technique
allows a good control of the membrane structure, porosity and
electrochemical properties. Such properties were found to be
significantly affected by the presence of inorganic fillers. The
composite membranes with 0.2–0.5 wt% of SS showed the
optimum properties and performance in ED, which is compa-
rable to the commercial benchmark membranes. Incorporating
sulfonated mesoporous silica was shown to be an effective
approach to enhance the performance of ion-exchange
membranes. The findings from this work will lead to a better
understanding of the effects of inorganic fillers on sPES
membranes and provide new insights into how to develop
composite ion-exchange membranes with desirable properties for
desalination.
Acknowledgements
The financial support from Australian Research Council
(through its ARC Centre of Excellence and Discovery
programs), CSIRO Advanced Membranes for Water Treatment
Cluster Project, and Thai government (through Higher Educa-
tional Strategic Scholarship for Frontier Research Network) is
gratefully acknowledged. Additional thanks are due to Richard
and Robyn Webb for technical support on the SEM sample
preparation and TEM.
References
1 G. S. Gohil, R. K. Nagarale, V. V. Binsu and V. K. Shahi, J. ColloidInterface Sci., 2006, 298, 845–853.
2 J. Balster, O. Krupenko, I. Punt, D. F. Stamatialis and M. Wessling,J. Membr. Sci., 2005, 263, 137–145.
3 R. Scherer, A. M. Bernardes, M. M. C. Forte, J. Z. Ferreira andC. A. Ferreira, Mater. Chem. Phys., 2001, 71, 131–136.
4 M.-S. Kang, Y.-J. Choi, I.-J. Choi, T.-H. Yoon and S.-H. Moon, J.Membr. Sci., 2003, 216, 39–53.
5 A. Elattar, A. Elmidaoui, N. Pismenskaia, C. Gavach andG. Pourcelly, J. Membr. Sci., 1998, 143, 249–261.
6 Y. S. Dzyazko and V. N. belyakov, Desalination, 2004, 162, 179–189.7 S. Feng, Y. Shang, X. Xie, Y. Wang and J. Xu, J. Membr. Sci., 2009,335, 13–20.
8 H. K. Hansen, L. M. Ottosen and A. Villumsen, Sep. Sci. Technol.,1999, 34, 2223–2233.
9 C. Iojoiu, M. Marechal, F. Chabert and J.-Y. Sanchez, Fuel Cells,2005, 5, 344–354.
10 N. N. Krishnan, H.-J. Kim, M. Prasanna, E. Cho, E.-M. Shin, S.-Y. Lee, I.-H. Oh, S.-A. Hong and T.-H. Lim, J. Power Sources,2006, 158, 1246–1250.
This journal is ª The Royal Society of Chemistry 2011
11 G. Chamoulaud and D. B�elanger, J. Colloid Interface Sci., 2005, 281,179–187.
12 R. Marschall, I. Bannat, J. Caro and M. Wark, MicroporousMesoporous Mater., 2007, 99, 190–196.
13 R. Marschall, I. Bannat, A. Feldhoff, L. Wang, G. Q. M. Lu andM. Wark, Small, 2009, 5, 854–859.
14 H. Dai, R. Guan, C. Li and J. Liu, Solid State Ionics, 2007, 178, 339–345.
15 R. K. Nagarale, G. S. Gohil, V. K. Shahi, G. S. Trivedi andR. Rangarajan, J. Colloid Interface Sci., 2004, 277, 162–171.
16 I. S. Byun, I. C. Kim and J. W. Seo, J. Appl. Polym. Sci., 2000, 76,787–798.
17 J. Choi, K. M. Lee, R. Wycisk, P. N. Pintauro and P. T. Matherc, J.Electrochem. Soc., 2010, 157, B154–B159.
18 V. K. Shahi, Solid State Ionics, 2007, 177, 3395–3404.19 R. K. Nagarale,W. Shin and P. K. Singh,Polym. Chem., 2009, 1, 388–
408.20 L. Li and Y. Wang, J. Power Sources, 2006, 162, 541–546.21 C. L. Buquet, K. Fatyeyeva, F. Poncin-Epaillard, P. Schaetzel,
E. Dargent, D. Langevin, Q. T. Nguyen and S. Marais, J. Membr.Sci., 2010, 351, 1–10.
22 G. Alberti, M. Casciola, M. Pica and G. D. Cesare, Ann. N. Y. Acad.Sci., 2003, 984, 208–225.
23 V. V. Binsu, R. K. Nagarale and V. K. Shahi, J. Mater. Chem., 2005,15, 4823–4831.
24 R.-Q. Fu, L. Hong and J. Y. Lee, Fuel Cells, 2007, 1, 52–61.25 C. Li, G. Sun, S. Ren, J. Liu, Q. Wang, Z. Xu, H. Sun and W. Jin,
J. Membr. Sci., 2006, 272, 50–57.26 K. Miyatake, T. Tombe, Y. Chikashige, H. Uchida and M. Watanbe,
Angew. Chem., Int. Ed., 2007, 46, 6646–6649.27 S. P. Nunes, B. Ruffmann, E. Rikowski, S. Vetter and K. Richau,
J. Membr. Sci., 2002, 203, 215–225.28 C. Klaysom, R. Marschall, B. P. Ladewig, G. Q. M. Lu and L. Wang,
J. Mater. Chem., 2010, 20, 4669–4674.29 R. K. Nagarale, G. S. Gohil and V. K. Shahi, Adv. Colloid Interface
Sci., 2006, 119, 97–130.30 J.-H. Choi, S.-H. Kim and S.-H.Moon, J. Colloid Interface Sci., 2001,
241, 120–126.31 C. Klaysom, S.-H. Moon, B. P. Ladewig, G. Q. M. Lu and L. Wang,
J. Membr. Sci., 2011, 371, 37–44.32 M. Wilhelm, M. Jeske, R. Marschall, W. L. Cavalcanti, P. Tolle,
C. Kohler, D. Koch, T. Frauenheim, G. Grathwohl, J. Caro andM. Wark, J. Membr. Sci., 2008, 316, 164–175.
33 L. Chazeau, C. Gauthier, G. Vigier and J. Y. Cavaille, inHandbook ofOrganic–Inorganic Hybrid Materials and Nanocomposites, ed. H. S.Nalwa, American Scientific Publishers, 2003, vol. 2,Nanocomposites, pp. 63–111.
34 C. Barth, M. C. Goncalves, A. T. N. Pires, J. Roeder and B. A. Wolf,J. Membr. Sci., 2000, 169, 287–299.
35 J. Barzin and B. Sadatnia, Polymer, 2007, 48, 1620–1631.36 A. Conesa, T. Gumi and C. Palet, J. Membr. Sci., 2007, 287, 29–40.37 P. Van de Witte, P. J. Dijkstra, J. W. A. Van de Berg and J. Feijen,
J. Membr. Sci., 1996, 117, 1–31.38 A. Noshay and L. M. Robeson, J. Appl. Polym. Sci., 1976, 20, 1885–
1903.39 J. Balster, M. H. Yildirim, D. F. Stamatialis, R. Ibanez,
R. G. H. Lammertink, V. Jordan and M. Wessling, J. Phys. Chem.,2007, 111, 2152–2165.
40 R. Ibanez, D. F. Stamatialis and M. Wessling, J. Membr. Sci., 2004,239, 119–128.
41 N. Pismenskaya, P. Sistat, P. Huguet, V. Nikonenko andG. Pourcelly, J. Membr. Sci., 2004, 228, 65–76.
42 V. M. Aguilella, S. Mafe, J. A. Manzanares and J. Pellicer, J. Membr.Sci., 1991, 61, 177–190.
J. Mater. Chem., 2011, 21, 7401–7409 | 7409